A container initially has 5.82 moles of N,0, 8.14 moles of O,, and 1.03 moles of N,0, in a box. Assume that the only reaction that can occur in this box is the one represented by the following balanced chemical equation: 2 N,0(g) + 3 02(g) 2 N,04(g) How many moles of N204 will be present in the box if (only) 5.00 moles (of the original 5.82 moles) of N20 react according to the equation above.

Which one of the following represents a combination reaction?   C2H4(g) + H2(g) → C2H6(g)       Fe(NO3)2(aq) + Na2S(aq) → FeS(s) + 2 NaNO3(aq)       Cr(s) + Pb(NO3)2(aq) → Cr(NO3)3(aq) + Pb(s)       2 KClO3(s) → 2 KCl(s) + 3 O2(g)

Be sure to answer all parts. Some coal is high in sulfur (S) content, and when it burns, it forms sulfuric acid (H,SO,), a major component of acid rain, by a series of reactions. Balance the equation for the overall conversion drawn below. s) + 0,(g) + H,O() → H,SO,(ag)

2NO(g) + O2(g) → 2NO2(g) You are provided with 4.12 molmol of nitrogen monoxide gas. Using the balanced chemical equation completed in Part A, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen dioxide are formed as a result? Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.80 molmol   NH3 and 4.64 mol O2 react. Express the amounts in moles to two decimal places separated by a comma.

Balance the equation below. CO(g) + O2(g) → CO2(g) How many moles of CO(g) are required to react completely with 1 mole of O2(g)? Enter your response in moles (mol) to the nearest 0.1 mol.

O = rosoft C W There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(1) oxide and sulfur dioxide: 2Cu₂S (s) + 30₂(g) → 2Cu₂0(s) + 2 SO₂ (g) In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: Cu₂O(s) + C(s)→ 2Cu(s) + CO (g) Microsoft O CHEMICAL REACTIONS Reaction sequence stoichiometry Microsoft 6.52.210... esc Suppose the yield of the first step is 64.% and the yield of the second step is 88.%. Calculate the mass of oxygen required to make 2.0 kg of copper. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. Explanation aption Q A T N 11 2 Check 9,039 W S X command #3 E 010 14 4 X $ C DEC 3 R F Ś % 5 V T útv G () > Y Ø 7 H Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibil 917 C N * 00 8 J FERBARKE I A M -0 K O L 28 W command

Given the unbalanced equation CO2 + H2→ CH4 + H2O   (a) How many moles of water can be produced from 37 moles of carbon dioxide?   (b) How many moles of CH4 will be produced along with 14 moles of water?

What is the sum of coefficients from the following reaction (both products and reactants)? X(CO3)3 + Heat ---> X can be any element. (Question 19)

Consider the reaction: 2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H₂(g) If a sample of 4.0 moles of Al is added to a solution containing 2.0 moles of HCI, how many moles of AICI3 are formed? O 4.0 moles 6.0 moles 0.67 moles 2.0 moles O 1.0 moles MacBook Air

Calculate the mass(in grams) of the product formed when 15.40g of  Cl_2(g) completely reacts. Assume that there is more than enough of the other reactant. 2 K(s) + Cl _2(g) --> 2KCl(s)