2 days ago

An unknown compound is composed of 65.44% C, 29.07% O, and 5.49% H. A sample weighing 5.34 g, when dissolved in 60.00 g H2O, low

ers the freezing point to -0.600°C. What is the molecular formula of the compound? (Kf for water = 1.86°C/m; C = 12.0, O = 16.0, H = 1.0 g/mol). A) C7H5O3 B) CHO C) C14H11O6 D) C3H3O E) C5H5O5'

Chemistry

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VMariaS [2998]

Answer:

$m_{Mg}=30.8mgMg$

Explanation:

Greetings,

According to the provided chemical equation, the production of 31.2 mL of hydrogen allows one to calculate its moles using the ideal gas equation as detailed below:

$n_{H_2}=\frac{PV}{RT}=\frac{754torr*\frac{1atm}{760torr}*0.0312L}{0.082 \frac{atm*L}{mol*K}*298.15K}=1.27x10^{-3}molH_2$

Since the ratio of hydrogen to magnesium is 1:1, its milligrams are derived through the following proportional factor calculation:

$m_{Mg}=1.27x10^{-3}molH_2*\frac{1molMg}{1molH_2}*\frac{24.305gMg}{1molMg}*\frac{1000mgMg}{1gMg}\\m_{Mg}=30.8mgMg$

Regards.

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How many grams of calcium cyanide (Ca(CN)2) are contained in 0.79 mol of calcium cyanide?

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above shows a balloon full of gas which has a volume of 120.0ml at 300.0k assuming pressure remains constant , what is the voume

castortr0y [3046]

The balloon's volume is 128 ml when the gas temperature rises to 320.0 K. Explanation: Given the following: T1 (initial temperature) = 300K, V1 (initial volume) = 120ml, T2 (final temperature) = 320 K, V2 (final volume) =?. Pressure is kept constant during this process. From the equation: Given that the pressure stays constant, we have: V2 = Putting the values into this formula yields: V2 = 128 ml, which indicates the volume of the gas when the temperature increases from 300 K to 320 K.

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2 months ago