At room temperature, two identical rigid containers are separated and filled up with the equivalent to 200 mol of Ar in one, and 200 mol of O2 in the other. Select the INCORRECT statement. Oa. The density of the gases will be different. O b. For both gases to have the same mean velocity, we would need to cool down the container with O2. If the same amount of an inert gas is added to each container, both containers will show an identical C. surge of internal pressure. The container full of oxygen is heavier than the one full of argon. If the temperature is increased simultaneously to 60°C, both containers will show an identical surge of internal pressure. 35 An unknown compound consists of 78.50% Sn, 18.85% F, and 2.65% O. Find the molecular formula for the compound. Oa. SnOFo Ob Sn3OFs Oc Sn3O3F2 d. S12OF2 e. SNOF2

At room temperature, two identical rigid containers are separated and filled up with the equivalent to 200 mol of Ar in one, and 200 mol of O2 in the other. Select the INCORRECT statement. Oa. The density of the gases will be different. O b. For both gases to have the same mean velocity, we would need to cool down the container with O2. If the same amount of an inert gas is added to each container, both containers will show an identical C. surge of internal pressure. The container full of oxygen is heavier than the one full of argon. If the temperature is increased simultaneously to 60°C, both containers will show an identical surge of internal pressure. 35 An unknown compound consists of 78.50% Sn, 18.85% F, and 2.65% O. Find the molecular formula for the compound. Oa. SnOFo Ob Sn3OFs Oc Sn3O3F2 d. S12OF2 e. SNOF2

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

a cylinder is filled with 10.0 l of gas and a piston is put into it. The intitial pressure of the gas is measured to be 268. kPa. The piston is now pulled up, expanding the gas, until the gas has a final volume of 77.0L. Calculate the final pressure of the gas. Round your answer to 3 signifficant digits.
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the CO₂ gas evolved by a certain chemical reaction taking place at 40.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 87.0 mL. collected gas X water chemical reaction Sketch of a gas-collection apparatus Calculate the mass of CO₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. BEET Ar B
collected Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. gas chemical reaction water Suppose the 0, gas evolved by a certain chemical reaction taking place at 50.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 58.2 mL. Sketch of a gas-collection apparatus alo Calculate the mass of O, that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. ? Explanation Check © 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility
Calculate the mole fraction of each gas in a mixture of 43.6 g Xe and 36.8 g Kr. Show your work. Answer using complete sentences. H. = = = в I m冊A Enter your answer here 300 words left
1. A 2.00L flask contains Ar(g) at 752mmHg and 35oC. A 0.728g sample of C6H6(g) is added. A. Calculate the total pressure in the flask. B. What is the mole fraction of Ar(g)?
Sometimes in Io we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. collected gas Suppose the O, gas evolved by a certain chemical reaction taking place at 30.0 °C is collected over water, using chemical reaction water an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 44.8 mL. Sketch of a gas-collection apparatus ab Calculate the mass of O, that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center | Accessibility 6:20 AM N 35°F Mostly cloudy ENG 1/23/2022 Pll 26 506 F90 T. 4. R] T Y D F
An unknown compound is 53.5% C, 11.2% H, and 35.5% O. A. Determine the empirical formula. B. If a 2.35g gaseous sample of this compound occupies 565mL at 875mmHg and 30.0oC, what is the molar mass of this compound? C. Determine the molecular formula of this gas.
Q.28. Consider a gas mixture of nitrogen (N2) and methane (CH.) of total mass 80g. 31.14% of the total mass is nitrogen. The nitrogen is occupying a volume of 0.995 liters at 150 C. 1/ Calculate the total pressure of the gas mixture. 2/ Calculate the partial pressures of each gas.
#4
Please help with b-d
Calculate the mass
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the H, gas evolved by a certain chemical reaction taking place at 35.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 59.7 ml... collected ga water chemical reaction Sketch of a gas-collection apparatus Calculate the mass of H, that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases.