Which of the following expressions show the mathematical relationship between the quantities in separate conditions, according to Charles' Law? VP1 = V2P2 V,T1 = V2T2 O V,T, = V2/T2 O V/P1 = V½/P2

Organic Molecules Assignment Check © 2023 McGraw Hill LLC. All Rights Reserved. Draw the alkane formed when the following alkene is treated with H₂ in the presence of a Pd catalyst. Save For Later 8 Terms of Use | Privacy Center | Accessibility = 9 = 10 B fmm E

Consider the following balanced equation. 2 Sb (s)  +   3 H2O (g)    →   Sb2O3 (s)   +   3 H2 (g) 5.0 L of H2O gas, with a pressure of 1.29 atm and a temperature of 96.7 °C reacted. How many mol of Sb2O3 were formed? Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, liters = L, atmospheres = atm   What temperature (with proper s.f.) is entered into the equation? Enter the value in the first blank and the units in the second blank.     Calculate the mol of H2O reacted (enter value only, with proper s.f.).  mol   Use the three blanks to enter the number, unit, and substance (in this order) that appears in…

X consists of a fl exible container with eight particles of a gas as shown. What happens to the pressure of the system when X is converted to the representations in parts (a), (b), and (c)?

Starting with Charles's law (stated as an equation), obtain an equation for the final volume of a gas from its initial volume when the temperature is changed at constant pressure. From Charles's law, VT = constant Because this is true for initial conditions as well as for final conditions, we can write V. V; T T; Thus, the equation for the final volume is P.V = P;V; Drag and drop your selection from the following list to complete the answer: P T; V, = V, x Pr PV = constant V = constamt T VT = V;T, V, = V, x T = constant V. P;V; P V, = V, x P, PV = constant T T

A gas with an initial pressure of 1.33 atm at 85 ∘C is cooled to − 29 ∘C. Express the pressure to three significant figures and include the appropriate units.

Consider the following balanced equation. 2 Sb (s)  +   3 H2O (g)    →   Sb2O3 (s)   +   3 H2 (g) 5.0 L of H2O gas, with a pressure of 1.29 atm and a temperature of 96.7 °C reacted. How many mol of Sb2O3 were formed? Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, liters = L, atmospheres = atm   What temperature (with proper s.f.) is entered into the equation? Enter the value in the first blank and the units in the second blank.     Calculate the mol of H2O reacted (enter value only, with proper s.f.).  mol   Use the three blanks to enter the number, unit, and substance (in this order) that appears in…

Find the density of Freon-11 (CFC13) at 110.0 °C and 6.87 atm. Be sure your answer has the correct number of significant figures. Note: Reference the Fundamental constants table for additional information. g L 0x1.8 X

One of the steps to sweeten sour gas using the Claus process is reacting hydrogen sulfide gas with sulfur dioxide gas to produce water vapour and sulfur. 8.43 kL of hydrogen sulfide at 175 kPa and 250 °C reacts with excess sulfur dioxide. Calculate the mass, in kg, of sulfur produced.Do not show your work in the space provided.Record only your final answer with the correct number of significant digits and the proper units.

The partial pressure of the hydrogen gas collected is 0.928 bar. If the total volume of gas collected is 726 mL , what mass of hydrogen gas is collected? The molar mass of hydrogen gas is 2.016 g · mol Express your answer in grams to three significant figures. Πνα ΑΣφ MH2 g