when the oxide of arsenic is heated it sublimes and becomes a gas. at 650oc and a pressure of 690mmHg the 0.927g sample of the oxide has a volume of 194cm3.

calculate the volume,in cm3, that the sample would have at the same temperture (650oc) but at a pressure of 760mm Hg

P1V1 = P2V2
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To calculate the volume, V2, at the second pressure (760 mmHg) at the same temperature (650°C), we can use the equation P1V1 = P2V2, and solve for V2.

Given values:
P1 = 690 mmHg (initial pressure)
V1 = 194 cm^3 (initial volume)
P2 = 760 mmHg (final pressure)

Using the equation P1V1 = P2V2, we can rearrange it to solve for V2:

V2 = (P1V1) / P2

Substituting in the values we have:
V2 = (690 mmHg * 194 cm^3) / 760 mmHg

To simplify, we can convert units:
1 mmHg = 1 cmHg (since 1 mm = 0.1 cm)
V2 = (690 cmHg * 194 cm^3) / 760 cmHg

Now, we can calculate V2:

V2 = 176,460 cm^4 / 760 cmHg
≈ 232 cm^3

Therefore, the sample would have a volume of approximately 232 cm^3 at the same temperature (650°C) but at a pressure of 760 mmHg.