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Cyclopropane gas is 85.7 % C and 14.3 % C H by mass and has a density of 1.71 g/L at 755 mm Hg and 25C. a) What is the molar mass of cyclopropane? b) What is the chemical formula for cyclopropane?
Predict the sign of Delta Ssys for EACH of the following processes. -Gaseous Cl2 in the stratosphere to form gaseous Cl atoms. -Gaseous CO reacts with gaseous H2 to form liquid methanol, CH3OH. -Calcium phosphate precipitates upon mixing Ca(NO3)2(..
Assume the radius of a neutron to be approximately 1.0; times ;10^{ - 13} {rm cm}, and calculate the density of a neutron.
The element bromine at room temperature is a liquid with a density of 3.12g/ml calculate the mass of 125 ml of Bromine . What volume does 85.0 g of bromine occupy?
A solution that is made by combining 125mL of 0.050 M hydrofluoric acid with 50.0mL of 0.10 M sodium fluoride.
Consider the following reaction. N2(g) + 3H2(g) > 2NH3(g) The initial pressures of the H2 IS 3 atm and the pressure of the N2 IS 2 atm. Which statement is true? N2 is a limiting reagent H2 is a limiting reagent Neither gas is a limiting reagent
A 613-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 11.1g CO2 . What was the concentration of the HCl solution
What is the standard free energy change (kJ) for the following reaction at 499.0 K ? [Note: Answer should be expressed as "xxx.x", or with one sig fig after the decimal
Calculate the volume of 8.0g of oxygen gas if it has a temperature of 552 K, and a pressure of 5 atmosheres
Consider the dissolution of magnesium (s) in an aqueous hydrochloric acid solution. What minimum amount of 1.85 M hydrochloric acid is nessecary to produce 28.5 L of hydrogen at STP
Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH solution. Calculate the pH for the following.
A 4.50-g sample of LIL at 25.oC dissolves in 25.0 mL of water also at 25.0C. The final equilibrium temperature of the resulting solution is 60.8C. What is the enthalp of solution of LICL expressed in kilojoules per mole?
An experiment requires 40.0 of ethylene glycol, a liquid whose density is 1.114 . Rather than weigh the sample on a balance, a chemist chooses to dispense the liquid using a graduated cylinder. What volume of the liquid should he use?
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