Calcium carbide, CaC₂, reacts with water to produce acetylene gas, C₂ H₂. [Review Topics] Submit Answer [References] CaC₂ (8) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)2 (8) What volume of acetylene at 29 °C and 1.25 atm is generated by the complete reaction of 4.08 g of calcium carbide? Volume= L What volume would this quantity of acetylene occupy at STP? Volume = L Retry Entire Group 8 more group attempts remaining E Course Home

Calcium carbide, CaC₂, reacts with water to produce acetylene gas, C₂ H₂. [Review Topics] Submit Answer [References] CaC₂ (8) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)2 (8) What volume of acetylene at 29 °C and 1.25 atm is generated by the complete reaction of 4.08 g of calcium carbide? Volume= L What volume would this quantity of acetylene occupy at STP? Volume = L Retry Entire Group 8 more group attempts remaining E Course Home

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...

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If 7.68 gram of phosphorous solid is mixed with 1.00 L of Chlorine gas at STP to form P2Cl5 according to the following unbalanced chemical reaction P4 (s) + Cl2 (g) →P2Cl5 (g) The molar mass of P4 is 123.88 g/mol. The molar mass of P2Cl5 is 208.22 g/mol. D)Calculate the volume of the product. E) Calculate the pressure of the product.
[5] Sodium chlorate decomposes on heating to sodium chloride and oxygen gas. heat 2NACIO:(s) → 2NaCI(s) + 302(g) A 0.8765 g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 ml at a temperature of 22 °C and a pressure of 734 torr. Calculate the mass percent of NaCIO3 in the original sample. (At 22 °C the vapor pressure of water is 19.8 torr.)
A sample of sodium metal is added to water and the hydrogen gas evolved is collected in a gas measuring tube over water. The equation for the reaction is 2 Na (s) + 2 H₂O (1)→ 2 NaOH (aq) + H₂(g) If 95.0 mL of hydrogen are collected at 27 °C and 0.974 atm, what mass of sodium reacted?
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On our campus, there are approximately 30.000 students who use 2.5 x 10° kJ of energy per day. Suppose all of that energy comes from the combustion of a carbon- hydrogen-oxygen compound in the presence of excess O2(g). 2.647 g sample of this gaseous carbon-hydrogen-oxygen compound that occupies a volume of 580 mL at 918,6 Torr and 24.00 °C. The products of the combustion of the given amount are 5.059 g CO2(g), 3.106 g H2O(1), and enough heat to raise the temperature of the calorimeter assembly from 24.00 to 38.33 °C. What is the molecular formula of this unknown compound and how many kilograms of this compound are needed to provide enough daily energy to all students on campus? (The heat capacity of the calorimeter is 4.915 kJ/°C.)
P1A.12* Balloons are still used to deploy sensors that monitor meteorological phenomena and the chemistry of the atmosphere. It is possible to investigate some of the technicalities of ballooning by using the perfect gas law. Suppose your balloon has a radius of 3.0 m and that it is spherical. (a) What amount of H₂ (in moles) is needed to inflate it to 1.0 atm in an ambient temperature of 25 °C at sea level? (b) What mass can the balloon lift (the payload) at sea level, where the mass density of air is 1.22 kg m? (c) What would be the payload if He were used instead of H₂?
Water can be decomposed by electrolysis to hydrogen gas and oxygen gas. If 2.33 g of water is decomposed to H2(g) and O2(g) and the gases are collected in a 1.00 L flask over water at 25°C (vapor pressure H2O(l) = 23.8 mm Hg), what is the pressure in the flask?
When ozone (O3) is placed in contact with dry, powdered KOH at –15°C, the red-brown solid potassium ozonide (KO3) forms, according to the following balanced equation: 5 O3(g) + 2 KOH(s) → 2 KO3(s) + 5 O2(g) + H,O(s) Calculate the volume of ozone needed (at a pressure of 0.134 atm and – 15°C) to produce 4.69 g KO3.
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