Concept explainers
The equation for the reaction of iron and oxygen gas to form rust (
a. How many kilojoules are released when 2.00 g of Fe reacts?
b. How many grams of Fe203 form when 150 kJ are released?
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Basic Chemistry
- The number of moles of H2O produced in reaction of 50 mL 1.0 M HCl and 50 mL 1.0 M NaOH: (5.00×10−2) Joules released per mole of water formed: ?arrow_forwardNitroglycerine is a powerful explosive forming N2, O2, CO2 and H2O vapor when detonated. In addition, 6.26 kJ of heat is given off per gram of nitroglycerine detonated. A) Balance the equation shown below. C3H5(NO3)3 (l) yields N2 (g) + O2 (g) + CO2 (g) + H2O (g) , delta H =? B) What is the delta H (kJ/mol) of nitroglycerinearrow_forwardIn the "Méthode Champenoise," grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is C,H12Os (aq) + 2C, H;OH(aq) + 2002(9) Fermentation of 893 ml grape juice (density is 1.0 g/cm') is allowed to take place in a bottle with a total volume of 971 mL until 15% by volume is ethanol (C,H; OH). Assuming that CO2 obeys Henry's law, calculate the partial pressure of CO, in the gas phase and the solubility of CO, in the wine at 25°C. The Henry's law constant for CO, is 3.1 x 10-2 mol/L atm at 25°C with Henry's law in the form C = kP, where C is the concentration of the gas in mol/L. (The density of ethanol is 0.79 g/cm.) (Enter your answers to two significant figures.) Partial pressure atm Solubilityarrow_forward
- Write a balanced chemical equation based on the following description: butanoic acid, C,H;COOH(I) burns in air C,H,COOH(I) + 5 0,(g) → 4 CO;(g) + 4 Hz0(1) O2+ 3+ 04- 2. O4+ 1 4. 8. 6. 02 O3 O5 O6 O8 09 (s) (1) (g) (aq) %3D C. OX H. H. Reset Delete w/ 口 3. 2.arrow_forwardWater can undergo a decomposition reaction, as shown in the following balanced equation. 2H2O(g) → 2H2(g) + O2(g) How many grams of oxygen gas O2 will be formed by the decomposition of 72.0 g of water vapor (H2O)? Show all work. (5 marks) (1) balance equation, list Givens, and Molar mass (M) 2 H2O(g) → 2 H2(g) + O2(g) m = 72.0 g _______ = m M = _______ _______ = M n = _______ _______ = n (2) convert mass of given (m) to amount of given (n) ***Use molar mass (M) (3) convert the amount of given (n) to the amount of required. ***Use mole ratios (4) convert the amount of required substance to required mass ***Use molar mass (M)arrow_forwardThe burning of iron pyrites (FeS.) in air may be expressed by the following reaction: Fes2 + 02 -> Fe203 + SO2 а. What mass of iron pyrite must be burned in air to produce 400.0g of ferric oxide? (8) b. What mass of oxygen will be consumed? ( C. How many molecules of sulfur dioxide will be produced ?arrow_forward
- Part I. Complete the following chemical reactions. Do not forget to balance the reaction, the states of matter and answer any questions that are asked. In the next reaction, a gas is formed. (19 points). HCl (aq) + Mg (s) → Gas that was released: Mg (s) + O2 (g) → Cu2S (s) + O2 (g) → Gas that was released:arrow_forward2. The reaction of between hydrazine (N₂H₁) and dinitrogen tetroxide (N₂0₂) in their liquid form is used to propel rockets into the air. 2N₂H4(1) + N₂04(1) 3N2(g) + 4H₂O(g) Substance N₂H4(1) N₂O4(1) N₂(g) H₂O(g) 9.16 0 -241.83 ΔΗ°,(kJ/mol) AS (J/mol.K) 50.6 121.2 304.3 191.5 188.72 Calculate the AH, AS, and AG. Is the reaction spontaneous at standard conditions?arrow_forwardIn an experiment, 7.84 g of sulphuric acid reacts with potassium carbonate. H2SO4 + K2CO3 —> K2SO4 + H2O + CO2 Calculate: the mass of potassium carbonate consumed (11.0g)arrow_forward
- Butane, C4H10, is flammable and used in butane lighters. What is the coefficient of oxygen in the balanced equation for the combustion of butane?__C4H10(g) + __O2(g)=> __CO2(g) + __H2Oarrow_forwardBalance the following chemical equation (if necessary): C,H(g) + O,(g) –→ H̟O(g) + CO,(g) 04- 3. D2+ 3+ O4+ 1 4 6. 8. 9. 9. (s) (1) (g) (aq) CH0 CO, H̟O Reset • x H,O Delete 5arrow_forwardThe reaction between potassium chlorate and red phosphorus takes place when you strike a match on a matchbox. If you were to react 52.9 g of potassium chlorate (KCIO,) with excess red phosphorus, what mass of tetraphosphorus decaoxide (P,O10) would be produced? KC1O:(5) + P4(s) - P,O0(5) + KCI(s) (unbalanced)arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning