|Decaborane, BH14, was used as a fuel for rockets inthe 1950s. It reacts violently with oxygen, O to pro-B.O3 and water. Calculate the percentage bymass of BH14 in a fuel mixture designed to ensurethat B1oH14 and O2 run out at exactly the same time|(Such a mixture minimizes the mass of fuel that arocket must carry.)

The balanced chemical reaction between decaborane (B10H14) and oxygen (O2) can be written as…

Answered: |Decaborane, BH14, was used as a fuel…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.70PAE

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In 1774, C. Scheele obtained a gas by reacting pyrolusite (MnO2) with sulfuric acid. The gas, which had been obtained that same year by Joseph Priestley by a different method, was an element, A. (a) What is the element isolated by Scheele and Priestley? (b) Element A combines with almost all other elements. For example, with cesium it gives a compound in which the mass percent of A is 19.39%. The element combines with hydrogen to give a compound with a mass percent of element A of 94.12%. Determine the formulas of the cesium and hydrogen compounds. (c) The compounds of cesium and hydrogen with element A react with one another. Write a balanced equation for the reaction.
How many grams of gaseous ammonia will the reaction of 3.0 g hydrogen gas and 3.0 g of nitrogen gas produce?
When calcium carbonate is heated strongly, it evolves carbon dioxide gas. CaCO3(s)CaO(s)+CO2(g) 25 g of CaCO3 is heated, what mass of CO2would be produced? What volume would this quantity of CO2 (CU at STP?
You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1. volume gas X + 2 volumes gas Y2 volumes compound I 2. volumes gas X + 1 volume gas Y2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
Solar winds composed of free protons, electrons, and particles bombard Earth constantly, knocking gas molecules outof the atmosphere. In this way, Earth loses about 3.0 kg of mat-ter per second. It is estimated that the atmosphere will be gone inabout 50 billion years. Use this estimate to calculate (a) the mass(kg) of Earth’s atmosphere and (b) the amount (mol) of nitrogen,which makes up 75.5 mass % of the atmosphere.
) During the last 30 years of rapid development in space exploration, many different rocket fuels have been tried. Two of these fuels are hydrogen and dimethylhydrazine. The equations for the reactions of these fuels are: 2H2(g) + O:(g) → 2H2O(1) (CH:);N2H2(g) + 40:(g) N2(g) + 4H>O(g) + 2CO:(g) AH = -576 kJ n I. AH =-1694 kJ moi II. Which fuel releases the greater amount of energy per gram? Show your working.
Wine open to the air turns sour over time due to oxidation of ethanol (molar mass 46 g/mole) to acetic acid (molar mass 60.0 g/mole). The reactions are shown by these two equations. 2C,H,OH(aq) + O2(g) 2CH;CHO(aq) + 0,(g) 2CH,CHO(aq) + 2н,0() 2CH;COOH(aq) If there is a 40.0% yield for the first step and a 40.0% yield for the second step, how many grams of acetic can are produced if you start with 16.00 g of ethanol? A) 2.23 B) 3.34 g C) 44.5g D) 16.0 g
Hydrazine, N2H4, can be used as fuel to orient and maneuver spacecraft. The energy used to do so is obtained by reacting the hydrazine with dinitrogen tetroxide to form nitrogen gas and water vapor. Write and balance the chemical equation for this reaction.The spy satellite US-193 had 453 kg of hydrazine on board when it was destroyed. What mass of dinitrogen tetroxide would have had to be on board in order to completely react with the hydrazine? This reaction is a redox reaction. Assign oxidation states to each atom in the reaction,identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent. Answer in full please.
ge-R x 21/FA-CHM-121-08 General Che * OWLv2 | Online teaching and lea G how to find mass percent - Goo x + mengagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locator=assignment-take A sample of gas mixture from a neon sign contains 5.12 x 10 mol Ne and 4.40 × 10¬4 mol Kr. What are the mass percentages of Ne and Kr in the gas mixture? Mass percentages of Ne = Mass percentages of Kr = Submit Answer Try Another Version 6 item attempts remaining

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