Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas, C2H2, and solid calcium hydroxide were formed by the reaction of calcium carbide, CaC2, with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons.(a) Outline the steps necessary to answer the following question: What volume of C2H2 at 1.005 atm and 12.2 °C is formed by the reaction of 15.48 g of CaC2 with water?(b) Answer the question.

The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes of nitrogen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid sodium azide (NaN) into solid sodium and gaseous dinitrogen. 2. Suppose 84.0 L of dinitrogen gas are produced by this reaction, at a temperature of 19.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must have reacted. Round your answer to 3 significant digits. 미미

The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes of nitrogen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid sodium azide (NaN,) into solid sodium and gaseous dinitrogen. alb Ar 2. Suppose 12.0 L of dinitrogen gas are produced by this reaction, at a temperature of 13.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must have reacted. Round your answer to 3 significant digits. Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Accessibility <. lenovo dle WebEx at 3pm (dia' just before 3pm) Resp L-650-479-3208 Access Code (meeting Number): 737 129 915 Dois, 3134

A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder tha measures 52.0 cm wide and 62.4 cm high. The maximum safe pressure inside the vessel has been measured to be 7.00 MPa. For a certain reaction the vessel may contain up to 25.8 kg of sulfur hexafluoride gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Round your answer to 3 significant digits. temperature: C x10 X

A sample of propane is placed in a closed vessel together with an amount of O2 that is 3.05 times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole fraction of each component in the resulting mixture after oxidation assuming the H2O is a gas.

Upon heating 134 g MgSO4 · 7 H2O:(a) how many grams of water can be obtained? (b) how many grams of anhydrous compound can be obtained?

The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes of nitrogen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid sodium azide (NaN) into solid sodium and gaseous dinitrogen. dlo 2. Suppose 12.0 L of dinitrogen gas are produced by this reaction, at a temperature of 13.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must have reacted. Round your answer to 3 significant digits. Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use| Privacy | Accessibility > Activity Details You have viewed this topic MacBook Air 4) DI DD F10 F11 F9 F2 F3 F4 F1 10 #3 $ & 3. 4. 6. 8 9.

A sample of 3.42 mol of xenon is confined at low pressure in a volume at a temperature of 86 °C. Describe quantitatively the effects of each of the following changes on the pressure, the average kinetic energy per molecule in the gas, and the root-mean-square speed. (a) The temperature is increased to 199 °C (b) The volume is tripled. (c) The amount of xenon is decreased to 1.87 mol Give each answer as a decimal factor of the form: new value factor old value. A factor of 1 means no change. ChangeP KEavgms

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

Predict the volume of oxygen (at 25 degrees Celsius and 743 mm Hg) that will be liberated if 1.00g of sodium peroxide reacts with excess water via the following: 2Na2O2 (s) + 2 H2O (l)--> O2 (g) + 4 NaOH (aq)