Please answer correctly, due soon. Thank you. Unit 15 Homework10/14 answeredHomework • Due in 2 hoursHomework • UnansweredCorrectly identify the reactants and products in this reaction by matching each species (on the left) with its appropriate acid-base term (on the right).NH3 + H2CO3 = HCO,' + NHDrag and drop options on the right-hand side and submit. For keyboard navigation. SHOW MORE VNH3conjugate acidH,CO3baseHCO,acidNH+1=conjugate base[3 FullscreenV O 9:47IIIIII Unit 14 Homework6/12 answeredHomework • Due in 2 hoursU14 HW Question 3Homework • UnansweredHow will the system respond to an increase in temperature?S(s) + 02(8) = SO2(g)AH° < 0Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer.ashift leftbshift rightno changeUnansweredSubmit{3 Fullscreen

Given, a chemical reaction as follows, NH3+H2CO3⇌HCO3-+NH4+we are asked to identify the acid, base,…

Correctly identify the reactants and products in this reaction by matching each species (on the left) with its appropriate acid- base term (on the right). NH3 + H2CO3 = HCO,'+ NH†1 Drag and drop options on the right-hand side and submit. For keyboard navigation. SHOW MORE V NH3 conjugate acid H;CO, base HCo, acid NH conjugate base II II II

Correctly identify the reactants and products in this reaction by matching each species (on the left) with its appropriate acid- base term (on the right). NH3 + H2CO3 = HCO,'+ NH†1 Drag and drop options on the right-hand side and submit. For keyboard navigation. SHOW MORE V NH3 conjugate acid H;CO, base HCo, acid NH conjugate base II II II

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.110PAE

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The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
In the reaction of two moles of gaseous hydrogen and one mole of gaseous oxygen to form two moles of gaseous water vapor, two moles of products are formed from three moles of reactants. If this reaction is done at 1.01 104 Pa (and at 0 C), the volume is reduced by 22.4 L. (a) In this reaction, how much work is done on the system (H2, O2, H2O) by the surroundings? (b) The enthalpy change for this reaction is 483.6 kJ. Use this value, along with the answer to (a), to calculate rU, the change in internal energy in the system.
Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume each peanut, with an average mass of 0.73 g, is 49% peanut oil and 21% starch; the remainder is noncombustible We further assume peanut oil is palmitic acid, C16H32O2, with an enthalpy of formation of 848.4 kJ/mol. Starch is a long chain of C6H10O5 units, each unit having an enthalpy of formation of 960 kJ.
A wad of steel wool (specific heat=0.45J/gC) at 25C is misplaced in a microwave oven, which later is accidentally turned on high. The oven generates microwaves of 13.5 cm wavelength at the rate of 925 moles of those photons per second. All of the photons are converted to high-heat energy, raising the temperature of the steel wool. Steel wool reacts explosively with the oxygen in the oven when the steel wool reaches 400.0C. If the steel wool explodes after 1.55 seconds, how many grams of steel wool were accidentally put into the oven?
Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25C and 1.00 atm is required to heat one gallon of water (d=1.00g/mL) from 25C to 98C ? The reaction for the combustion of butane (H f =125.6kJ/mol) is C4H10(g)+132 O2(g)4CO2(g)+5H2O(g)
Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substance
For the process H2O(l)H2O(g) at 298 K and 1.0 atm, H is more positive than E by 2.5 kJ/mol. What does the 2.5 kJ/mol quantity represent?
9.26 Gas furnaces have achieved impressive efficiency levels largely through the addition of a second heat exchanger that condenses water vapor that would otherwise escape out the exhaust system attached to the furnace. How does this process improve efficiency?
At what points in the Chapman cycle do photochemical reactions take place?
9.86 You make some iced tea by dropping 134 g of ice into 500.0 mL of warm tea in an insulated pitcher. If the tea is initially at 20.0°C and the ice cubes are initially at 0.0°C, how many grams of ice will still be present when the contents of the pitcher reach a final temperature? The tea is mostly water, so assume that it has the same density (1.0 g/mL), molar mass, heat capacity (75.3 J K-1 mol-1), and heat of fusion (6.0 kJ/mol) as pure water. The heat capacity of ice is 37.7 J K-l mol-l.
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
One mole of H2O(g) at 1.00 atm and 100.C occupies a volume of 30.6 L. When 1 mole of H2O(g) is condensed to 1 mole of H2O(l) at 1.00 atm and 100.C, 40.66 kJ of heat is released. If the density of H2O(l) at this temperature and pressure is 0.996 g/cm3, calculate E for the condensation of 1 mole of water at 1.00 atm and 100.C.