Calculate the number of pounds of CO, released into the atmosphere when a 13.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C,H,3, and that the density of gasoline is 0.692 g mL-. This assumption ignores additives. Also, assume complete combustion. 18 CO, released: lb

What is the sum of coefficients from the following reaction (both products and reactants)? X.3H2O + Heat ---> X can be any element.

1. Label each of the following reactions as combination (synthesis), decomposition, single replacement, or double replacement. Then complete and balance the following reactions. Reaction Type of reaction? Redox or nonredox? H2(g) + 02 (g) → K (s) + N2 (g) → C (s) + 02 (g) → H2CO3 (aq) → electrical current H₂O (1) 300°C Au2O3 (s) 300°C Ag2O (s) → NH3 (g) → Pb (s) + Cu(NO3)2 (aq) → Na (s) + HOH (1) -> BaBr2 (aq) + Na3PO4 (aq) → H2SO4 (aq) + NH4OH(aq) → Cl2 (g) + NaI (aq) → Na2S (s) + HCl(aq) → Fe (s) + 02 (g) →

A vehicle airbag uses a gas generator that contains a mixture of three compounds: NaN3NaN3 , KNO3KNO3 , and SiO2SiO2 . A series of three reactions is used to convert the highly toxic sodium azide, NaN3NaN3 , into N2N2 gas and harmless silicate glass. The nitrogen gas fills up the airbag, causing it to rapidly expand in a head‑on collision. Balance the reactions involved in the deployment of an airbag by inserting the appropriate coefficients. Reaction 1: 2NaN3(s)---->2Na(s)+3N2(g) Reaction 2: 10Na(s)+2KNO3(s)----> K2O(s)+5Na2O(s)+N2(g) Reaction 3: K2O(s)+Na2O(s)+2SiO2(s)----> K2O3Si(s)+Na2O3Si(s) The driver‑side airbag deploys when a SUV is in a head‑on collision. The airbag inflates to a volume of 70.0 L70.0 L and a pressure of 1.41 atm1.41 atm at 25.0 °C25.0 °C . Calculate the amount of NaN3NaN3 , in grams, that the manufacturer of the vehicle placed into the gas generator to produce this amount of nitrogen gas. Assume that the nitrogen gas behaves as an ideal gas and the…

What is the sum of coefficients from the following reaction (both products and reactants)? X.3H2O + Heat ---> X can be any element.

What is true for this chemical reaction: CO₂(g) + 4H₂(g) = CH₂(g) + 2H₂O(g)? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C Reaction Changes Homework Unanswered Due Today, 11:59 PM d AHrxn > 0; ASrxn > 0 AHxn 0 AHxn 0; ASxn < 0 Unanswered. 2 attempts left

Write.a balanced equation when hydrogen gas reacts with oxygen gas to produce gaseous water. HTML Editor

Oo.72. Subject  :- Chemistry

The following unbalanced equation illustrates the overall reaction by which the body utilizes glucose to produce energy: C6H12O6(s) + O2(g) → CO2(g) + H2O(l)   What is the conversion factor that allows for the calculation of moles of carbon dioxide based on moles of glucose?

||| O Microsoft O The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO3(s) + O₂(g) 2MnO₂ (s) + 2 CO₂(g) W O CHEMICAL REACTIONS Reaction sequence stoichiometry In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO₂ (s) + 4A1(s)→ 3Mn(s) + 2 Al₂O₂ (s) Microsoft esc Suppose the yield of the first step is 73.% and the yield of the second step is 86.%. Calculate the mass of manganese(II) carbonate required to make 1.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. G Microsoft 6.52.210... Explanation B ! Check 9,270 280 103 x10 HE X OCT 24 ロ・ロ Ś III E % LC ustv ♫ 6 2 & 7 9 © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility DZA 8 9 1/5 W 0 30 Simrat V + 11 ? olo Ar 2…