Oxygen for astronauts in space can be produced chemically using a solid fuel oxygen generator. The reaction takes place at 600 °C and is shown below. NaCIO:(s) + Fe(s) → 302(g) + NaCI(s) + FeO(s) What volume of O2 gas will be produced when 855 g of NACIO3 reacts with excess iron at a pressure of 3 atm?

Oxygen for astronauts in space can be produced chemically using a solid fuel oxygen generator. The reaction takes place at 600 °C and is shown below. NaCIO:(s) + Fe(s) → 302(g) + NaCI(s) + FeO(s) What volume of O2 gas will be produced when 855 g of NACIO3 reacts with excess iron at a pressure of 3 atm?

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

What volume of carbon dioxide gas (in mL) at 835 mm Hg and 37 °C can be produced when 2.4 g of CaCO3(s) are put into an Erlenmeyer flask containing 108 mL of 0.152 M HCl(aq) ?1 CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the CO₂ gas evolved by a certain chemical reaction taking place at 40.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 87.0 mL. collected gas X water chemical reaction Sketch of a gas-collection apparatus Calculate the mass of CO₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. BEET Ar B
etermine the total volume of all gases formed when 75.0 mL an explosive (C3H5(NO3)3 , d = 1.60 g/mL, molar mass = 227.10 g/mol) reacts according to the following reaction. Assume room temperature and pressure conditions. 4 C3H5(NO3)3(l) → 6 N2(g) + O2(g) + 12 CO2(g) + 10 H2O(g)
a 2.802g sample of an unknown pure metal (M) is added to a 0.2 L solution of 2 mol/L H2SO4(aq). The metal reacts with the acid until the metal is completely gone to form M3+(aq) ion in the solution and produces hydrogen gas that is collected. The hydrogen gas that is collected over water that is isolated from the reaction has a volume of 0.82 L at 25 degrees Celsius and a total pressure of 704.0 mmHg. How many moles of H2(g) are produced? Write a balanced equation for the reaction of M with H2SO4(aq). What is the identity of metal M?
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the CO₂ gas evolved by a certain chemical reaction taking place at 55.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 129. mL. g x10 177 Sketch of a gas-collection apparatus x collected gas Calculate the mass of CO₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. water chemical reaction
A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)
#14
Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnClą(aq) +H2(g) The product gas, H,, is collected over water at a temperature of 20 °C and a pressure of 755 mm Hg. If the wet H, gas formed occupies a volume of 6.66 L, the number of moles of Zn reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.
Acetylene, used in welding torches, can be produced by the reaction CaC2(s) + 2 H2O(l) → C2H2(g) + Ca(OH)2(aq). A student found that 4.00 g of CaC2(s) would produce 1.71 L of C2H2(g) at SATP. The percent error in the experiment was Question 18 options: A) 90.5% B) 10.5% C) 89.3% D) 9.53%
Hydrogen gas can be prepared by the reaction of zinc metal with dilute aqueous hydrochloric acid: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) How many moles of hydrogen would be produced in the reaction if 7.90 g of zinc reacts? What volume of H2 would be produced in this reaction under standard conditions (25°C and 1.013 x 105 Pa)?
A fictitious metal called Oscium (MM = 72.4 g· mol) reacts with nitrogen gas according to the following reaction: 6 Oc (s) + N2(g) → 2 OC3N(s) Part A How many moles of N2 gas would be present in 55.1 mL at STP? Express your answer using three significant figures. ? mol