If 0.215 g of an unknown element reacted with HCl and produced 97.5 mL of H2 gas

Question

If 0.215 g of an unknown element reacted with HCl and produced 97.5 mL of H2 gas in a 1.1 ratio, at a temperature of 25.0 degree C and under a barometric pressure of 0.988 atm, what would be the atomic weight of this element?(The water level inside the gas collecting tube (graduated cylinder) was even with the water level in the pneumatic trough and water vapor pressure at 25 degree is 0.0313 atm) Why must water vapor pressure be subtracted from the total pressure? Why do you add the pressure of the height difference to the pressure of the gas if it is below the water level of the through and subtract the pressure of the height difference to the pressure of the gas if it is above the water level of the trough?

Explanation / Answer

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•DALTON´S LAW.- includes the effect of humidity on the partial pressures of gases. The water vapor pressure does not follow Dalton's Law because it depends primarily on the temperature under normal atmospheric conditions. When the partial pressure (P) of a gas in a mixture where the water vapor present, the total barometric pressure system must be corrected before calculating the partial pressure of this gas is calculated. P = (PB - PH2O) (C) The maximum water vapor (PH2O) to a temperature of 37 * C partial pressure is 47 mmHg. In implementing this change in the law to ambient air temperature of 37 8C, barometric pressure of 760 mmHg, saturated steam (PH 2 O = 47 mmHg) and oxygen concentration of 21%, the calculation of the partial pressure of oxygen shows the following results: P = (PB - PH 2 O) (C) = (760-47) (0.21) = 149.7

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