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The atmospheric pressure at the summit of mount mckinley is 575 mmHg on a certain day. What is the pressure in atmospheres and in kilopascals?
Determine the partial pressure of each gas in a mixture of gases using Dalton's law of partial pressures
You have a 48.9 g sample of water at the temperature of -60.0 degrees celcius. How much energy is required to: a) heat the ice to 0 degrees celcius
volumetric flask and this solution becomes quite warm, but after it is permitted to return to room temperature, H 2 O is combined to total 500 mili litres of solution. Compute the pH of the final solution. ?
Using a solution prepared by adding 467 mL of 0.400 M silver nitrate with 421 mL of 0.503 M sodium phosphate then determines what is the silver ion concentration in? Ksp of silver phosphate = 2.8 × 10-18
A 1.30 g sample of dry ice is added to a 760 mL flask containing nitrogen gas at a temperature of 25.0 degrees Celcius and a pressure of 735 mmHg. The dry ice is allowed to sublime.
What unusual aspect of water is responsible for it unique characteristics as both a liquid and as a solid? Give examples of how this property of water would affect food systems during processing.
A 1.0-L buffer solution is 0.105M in HNO 2 and 0.145M in NaNO 2. Determine the concentrations of HNO 2 and NaNO 2 after addition of 1.4g NaOH.
A buffer is made up 0.24 M propanoic acid, CH3CH2COOH, a weak monoprotic acid, and 0.17 M of sodium propanoate, CH3CH2COONa. What is the pH of the solution.
when 56.6 g of calcium and 30.5 g of nitrogen gas undergo a reaction that has a 93.0% yield, what mass (g) of calcium nitride forms.
Compute the difference in pressure between CH4 and an ideal gas if 14.0 moles of gas are in a 6.00 litres tank at the temperature of 21.1 degree celsius . The van der Waals constants for CH4 are a =2.300 L^2 x atm/mol ^2 and b=0.0430 L/mol.
If 42.3 L of PH3 forms when 85.1L of H2 (g) reacts with 167.6 (g) of P4 at STP. What is the percent yield.
A sample of oxygen gas () was found to effuse at a rate equal to three times that of an unknown gas. The molecular weight of the unknown gas is __________ g/mol.
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