Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn(s) + H₂SO4(aq) → ZnSO4(aq) + H₂(g) In an experiment, 177 mL of wet H₂ is collected over water at 27°C and a barometric pressure of 765 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27°C is 26.74 torr. O 3.47 x 105 g O 347 g O 0.457 g Ⓒ 3.85 x 106 g O 457 g Submit Request Answer

Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn(s) + H₂SO4(aq) → ZnSO4(aq) + H₂(g) In an experiment, 177 mL of wet H₂ is collected over water at 27°C and a barometric pressure of 765 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27°C is 26.74 torr. O 3.47 x 105 g O 347 g O 0.457 g Ⓒ 3.85 x 106 g O 457 g Submit Request Answer

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 801.1 mL aqueous solution of 628.5 mM Na2S is combined with 100.0 mL of an aqueous HCl solution whose HCl concentration is not known. The reaction produces 4.126 L of H2S gas at a pressure of 1.00 atm and a temperature of 35.93∘C. There are sulfide ions still present in the solution after the reaction is complete. What was the concentration of HCl in the original HCl solution? Express your answer in units of molar (M) using at least three significant digits.
Sulfur dioxide reacts with oxygen in the presence of plati- num to give sulfur trioxide: 2 SO2(g) + O2(g) → 2 SO3(g) Suppose that at one stage in the reaction, 26.0 mol SO2, 83.0 mol O2, and 17.0 mol SO3 are present in the reaction vessel at a total pressure of 0.950 atm. Calculate the mole fraction of SO3 and its partial pressure.
The partial pressure of O2 in the atmosphere at sea level is 21.3 kPa. What is the partial pressure of O2 on the top of a mountain, where the atmospheric pressure is 89.7 kPa? [Atmospheric pressure at sea level is 101.3 kPa.]
Use your text or other reference to find the partial pressure of water at 25°C, 26°C, and 27°C and record those values.
73. A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2 O2, in the presence of a small amount of manganese catalyst by the reaction 2H2 O2 (aq) → 2H2O (g) + The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? (The vapor pressure of water at 24 °C is 23 mm Hg.)
A dilute solution of acetic acid produced by fermentation and oxidation of natural carbohydrates is called vinegar. If 48.6 g of acetic acid, CH3COOH , are dissolved in 65.3 g of water, what is the mole fraction of acetic acid? Atomic Mass: C=12.01 ; H=1.008 ; O = 16.0
Vessel A (volume 16.6 L) contains 30 g of hydrocarbon, and its pressure at 300 K is 1 atm.What is molecular weight of hydrocarbon ?