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compressed gas cylinder contains 1.00 x 10^3 g of argon gas. The pressure inside the cylinder is 2050 psi at a temperature of 18 C. How much gas remains in the cylinder if the pressure is decreased to 650 psi at a temperature of 26 C?
Calculate how many moles of nitrogen will be required to make 10.0 moles of NH 3 and calculate what is energy of each pulse If each pulse contains no of photons =1.20 x 10 18
Suppose 50 mL of 0.020 M Hydhrochloric acid solution was mixed to 50 mL of 0.20 M acetic acid solution (Ka of acetic acid, CH3COOH, = 1.8 x 10-5). Determine the approximate pH of the mixture.
If 6.0 moles of ethene and 6.0 moles of hydrogen are introduced into a 2.0 L sealed vessel and allowed to equilibrate at 200ºC, what is the equilibrium concentration of the ethene
How much heat energy would be needed to raise the temperature of a 15.0 g sample of iron (C = 0.448 J/goC) from 22.0 oC to 100.0 oC?
The evaporation of water H2O(l) ->H2O(g) is endothermic: Change in T degree +44.01 kJ Determine the minimum mass of water (in ) has to evaporate to absorb 183 joules of heat?
Would you help me to determine the term symbols allowed by the Pauli exclusion principle for the electron configuration 3d2 . Order the terms from lowest energy to highest.
methane and hydrogen sulfide form when 36g H2 reacts with carbon disufide. Calculate the percent yield if the actual yield of CH4 is 69.8
A compound of forumula C14H12 gave a positive Baeyer test and burned with a yellow, sooty flame. Treatment with ozone followed by hydrolysis in the presence of zinc gave formaldehyde as one of the products.
Draw a diagram showing the stratification in a body of water. Label the different layers and describe the type of chemistry (and species) that occurs at each level.
A gas has a volume of 590 mL at a temperature of -55.0C. What volume will the gas occupy at 30.0C.
1.60 M solution(78.0 mL ) is diluted to a volume of 278 mL and a 139-mL portion of that solution is diluted using 175 mL of H 2 O ,water determine the final concentration?
Calculating the molecular formula of an organic compound. Worked example, using fundamental formula and balanced equations.
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