Constants: R = 0.0821 atmL/molK, 760 mmHg = 1atm Copper (II) sulfıde dissolves in concentrated nitric acid according to the following reaction: 3CUS(s) + 8HNO3(aq) -----> 3CUSO4(aq) + 8NO(g) + 4H2O(1) What volume of NO(g) is produced at 1.2atm and 23°C if 45.7g of copper (II) sulfide and 230.mL of 5.00M of nitric acid solution (HNO3(aq)) are combined?

Constants: R = 0.0821 atmL/molK, 760 mmHg = 1atm Copper (II) sulfıde dissolves in concentrated nitric acid according to the following reaction: 3CUS(s) + 8HNO3(aq) -----> 3CUSO4(aq) + 8NO(g) + 4H2O(1) What volume of NO(g) is produced at 1.2atm and 23°C if 45.7g of copper (II) sulfide and 230.mL of 5.00M of nitric acid solution (HNO3(aq)) are combined?

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

Find the pressure in Torr of 0.0080 mol of an ideal gas contained in 125 L at 15 °C: R = 62.36 L·Torr/(mol·K)
For the following reaction: C3H8(g) + 3CO₂(g) + 4H₂O(1) 502(g) The change in gaseous moles, An = To maximize the product yield, the volume of the container should ◆ , so that the pressure will be (> →
An “empty" spray can contains residual propellant gas that has a pressure of 772 torr at 23°C. The can is then heated to 475 °C. (a) What is the gas pressure in the hot can if the volume remains constant? (b) What is the gas pressure in the hot can if the can slightly expands during heating and its volume increases by 6.50%?
I AM NOT A NATIVE ENGLISH SPEAKER, PLS WRITE IT CLEAR. The following is a formulation of the decomposition of penta-nitrogen dioxide in 456K N2O5(g) → 2NO2(g) +1\2O2(g) ? = 6.35 × 10−3?−1 A 0.18 liter hard vessel located in the 456K was inserted N2O5(G) At a pressure of 1.22 atmospheres. the reaction above happend. 1. How long from the start of the experiment will the pressure in the system rise to 1.54 atmospheres? 2. Calculate the partial pressure of each component in the mixture 100 seconds from the start of the experiment. 3. It was found that at a temperature of K 400 the value of the rate constant for a decomposition reaction of a nitrogen Fanta-oxygen equals 5.42*10-3 sec-1. Calculate the operating energy for the reaction. in all sections show calculations.
Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NaOH(aq) + 6H₂O2NaAl(OH),(aq) + 3H₂(g) In an experiment, the H₂ gas is collected over water in a vessel where the total pressure is 751 torr and the temperature is 25°C, at which temperature the vapor pressure of water is torr. If the wet H₂ gas formed occupies a volume of 7.02 L, the number of moles of H₂ 23.8 ton. Under these conditions, the partial pressure of H, is formed is mol.
[6] Magnesium carbonate reacts with hydrochloric acid to form the products shown below. If 45.0 g of MgCO; reacted with 50 ml of 0.1000M HCl what volume of CO2 would be produced at STP. MgCO3(s) + 2HCI (aq) → MgCl2(aq) + H2O(1) + CO2(g)
A gaseous “CFC” compound has a density of 5.456 g/L at 0.993 atmand 22.0oC. (a) Calculate the molar mass of the compound. (b) If the compound has the following composition: 18.10% C; 28.60% F, and 53.30% Cl, by mass, determine the molecular formula of the compound. (CFC = chlorofluorocarbon)
4.) (a) 0.375 g of CO2 gas is held in a 520.-mL container at 24. oC. What is its pressurre? atm (b) 0.375 g of N2 are held in an identical container at the same temperature. What is its pressure? atm (c) Are the pressures the same or different? Why? (d) If both these samples were contained in the same 520.-mL container, what would the partial pressure of each gas be? What would the total pressure be? (FYI, these gases do not react.) PCO2= atm PN2= atm…
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
A sample of gas contains 0.150 mol of N₂(g) and 0.300 mol of H₂(g) and occupies a volume of 21.4 L. The following reaction takes place: N₂(g) + 2H₂(g)-N₂H4(9) Calculate the volume of the sample after the reaction takes place (assume temperature and pressure are constant).
[References] Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H2O2(aq) → 2H2O(1) + O2(g) What volume of pure O2(g), collected at 25°C and 744 torr, would be generated by decomposition of 127 g of a 50.0% by mass hydrogen peroxide solution? Ignore any water vapor that may be present. Volume = L
Consider the reaction shown below: 2 HCl (aq) + CaCO3 (s) ⟶ CO2 (g) + CaCl2 (aq) + H2O (l) How many grams of CaCO3 would need to be consumed to fill a 908.001 mL balloon with CO2 gas, assuming a constant temperature of 21.7 oC and constant pressure of 0.958 atm? Express your answer in units of grams using at least three significant figures.