Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂ (s) + 2H₂O(1)→C₂H₂(g) + Ca(OH)₂ (aq) The product gas, C₂H₂, is collected over water at a temperature of 25 °C and a pressure of 758.0 mmHg. If the wet C₂H₂ gas formed occupies a volume of 6.92 L, the number of grams of C₂H₂ formed is g. The vapor pressureof water is 23.8 mm Hg at 25 °C.ĴCalcium carbide reacts with water to produce acetylene gas according to the following equation:CaC₂ (a) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)₂ (aq)The product gas,C₂H₂, is collected over water at a temperature of 25 °C and a pressure of 758.0 mm Hg. If the wetC₂H₂ gas formed occupies a volume of 6.92 L, the number of grams ofC₂H₂ formed isg. The vapor pressure of water is 23.8 mm Hg at 25 °C.

The ideal gas equation gives the relation between pressure, volume, temperature, and number of moles…

Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂ (s) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)₂ (aq) The product gas, C₂H₂, is collected over water at a temperature of 25 °C and a pressure of 758.0 mm Hg. If the wet C₂H₂ gas formed occupies a volume of 6.92 L, the number of grams of C₂H₂ formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C. Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂ (a) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)2 (aq) The product gas, C₂H₂. is collected over water at a temperature of 25 °C and a pressure of 758.0 mm Hg. If the wet C₂H₂ gas formed occupies a volume of 6.92 L, the number of grams of C₂H₂ formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C.

Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂ (s) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)₂ (aq) The product gas, C₂H₂, is collected over water at a temperature of 25 °C and a pressure of 758.0 mm Hg. If the wet C₂H₂ gas formed occupies a volume of 6.92 L, the number of grams of C₂H₂ formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C. Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂ (a) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)2 (aq) The product gas, C₂H₂. is collected over water at a temperature of 25 °C and a pressure of 758.0 mm Hg. If the wet C₂H₂ gas formed occupies a volume of 6.92 L, the number of grams of C₂H₂ formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C.

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

Given 2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20°C and a pressure of 759 mm Hg. If the wet H2 gas formed occupies a volume of 7.42L, how many grams of H2 are formed? The vapor pressure of water is 17.5 mm Hg at 20°C.
Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂ (s) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)2 (aq) The product gas, C₂ H2, is collected over water at a temperature of 20 °C and a pressure of 742.0 mm Hg. If the wet C₂2H2 gas formed occupies a volume of 9.02 L, the number of moles of CaC2 reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.
When zinc metal is added to hydrochloric acid, the following reaction takes place Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g) Calculate the volume of H₂ gas collected over water at 30.0 °C when 71.9 g of zinc is added to excess hydrochloric acid if the total pressure is 695 torr. The vapor pressure of water at 30.0 °C is 31.8 torr.
Use the ideal gas equation, PV = nRT, to calculate the volume in liters of 1.808 moles of nitrogen gas collected at 17.5°C and 760.22 mmHg. The gas was not collected over water. R = 82.1 atm·mL/mol·K or R = 0.0821 atm·L/mol·K
A 31.3 mL sample of an unknown, water-insoluble gas was collected over water at 20.4°C and a barometric pressure of 0.805 atm. When the gas was dried and chilled, it formed 103.14 mg of liquid. What was the molar mass of this substance? [The vapor pressure of water at 22.6°C is 20.0 mmHg]
For many purposes we can treat dimethyl ether C2H6O as an ideal gas at temperatures above its boiling point of −24.°C. Suppose the pressure on a 480.mL sample of dimethyl ether gas at 4.00°C is doubled. Is it possible to change the temperature of the dimethyl ether at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C.
in the following reaction, 27.1 mL of o2(g) is collected over water at 23*C and barometric pressure 751 mmHg. After the reaction, the buret could not be lowered far enough to make the water levels equal in both the burette and beaker. In fact, you measured the difference in water levels to be 34 mm, what must have been the mass of the Ag2O decomposed? (the vapor pressure of water at 23* C is 21.1 mmHg)
Elemental analysis of an organic liquid with a fishy odour gives the following elemental mass percentages: H 14.94 % C 71.22% N 13.84 %. Vaporization of 270 mg of an impure sample in a 150-mL bulb at 150oC gives a pressure of 435 torr. What is the molecular formula of the compound, and the % purity of the sample?
Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H20(1)2NAOH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 758 mm Hg. If the wet H2 gas formed occupies a volume of 7.27 L, the number of grams of H2 formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C.
Acetylene can be made reacting calcium carbide with water. CaC2 (s) + 2 H2O (l) →→ C2H2 (g) + Ca(OH)2 (aq) Assume that you place 2.65 g CaC2 in excess water and collect the acetylene over water. The volume of the collected gas is 795 mL at 25.0 °C and a barometric pressure of 735.2 mm Hg. Calculate the percent yield of acetylene. Note: the vapor pressure of water at 25.0 °C is 23.8 mm Hg.
A sample of oxygen is collected over water at 24°C and 757 mm Hg in a 125-mL flask. The vapor pressure of water at 24°C is 22.4 mm Hg. The partial pressure is 734.6 mmHg. There are 4.96x10^-3 moles of dry gas collected. If 0.0205g of N2(g) are added to the flask at the same temperature, the partial pressure of nitrogen in the flask is 108.7 mmHg. What is the total pressure in the flask after nitrogen is added?
For many purposes we can treat propane (C₂Hg) as an ideal gas at temperatures above its boiling point of -42. °C. Suppose the temperature of a sample of propane gas is lowered from 21.0 °C to -24.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.34 kPa and the volume decreased by 55.0%, what is the final pressure? Round your answer to the correct number of significant digits. kPa X Ś