Question 1 Calculate the amount of work done against an atmospheric pressure of

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Question 1 Calculate the amount of work done against an atmospheric pressure of 745 torr when 85.0 g of zinc dissolves in excess acid at 40.0 degree C. Given: R = 8.314 J/K*mol = 0.0821 L*atm/K*mol Question 2 In the following reaction, how many moles of the non-limiting reactant are in excess if 3.50 mol Al are combined with 3.60 mol HCl? Question 3 Consider the following reaction: If 9.0 L of C4H8 react with 9.0 L of O2, what is the volume of each gas ( C4H8 , O2 , CO2 , H2O), respectively, after the completion of the reaction? Question 4 A 2.55-mL sample of heptane, C7H16, is burned in an excess of oxygen gas in a carbon-hydrogen analyzer. What mass of water and how many liters of carbon dioxide at STP should be obtained? The density of heptane is 0.684 g/mL. Molar mass of heptane is 100.2 g/mol. Question 5 Two sucrose solutions. 125 mL of 1.50 M C12H22O11 and 275 mL of 1.25 M C12H22O11, are mixed Assuming the solution volumes are additive, what is the molarity of sucrose in the final solution? Question 6 How many milliliters of 0.1000 M H2SO4 are required to react with 10.32 mL of 0.4042 M NaHCO3? Question 7 A student needs 62.5 g of zinc sulfide, a white pigment, for an art project. He can synthesize it using the reaction: How many grams of zinc nitrate will he need if the percent yield of zinc sulfide is 85.0 %?

Explanation / Answer

1. (e) +3.38 kJ ( Assuming expansion work to be positive)

2. (c) 2.30 moles Al

3. (e) 7.5 l, 0.0 L, 6.0 L, 6.0 L

4. (d) 2.5g H2O; 2.72 L CO2

5. (b) 1.33 M

6. (b) 20.86 mL

7. (c) 143 g

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