If 14 grams of hydrogen reacted with 24.7 grams of oxygen 27.7875 grams of water will be formed.
Explanation:
2H2+O2----------->2H2O.
- From the above equation, we can say that 4g of Hydrogen will react with 32 g of oxygen.
- In this question, Hydrogen is in excess amount.
- 32 g of Oxygen will react with = 4 g of H2.
- Therefore 24.7g of Oxygen will react with =24.7x4/32= 3.0875 g H2.
- The remaining 10.9125g of H2 will be left unreacted.
- Therefore the amount of water formed=(24.7+3.0875)=27.7875 g
Answer:
Explanation:
The ideal gas law equation is an equation that relates some of the quantities that describe a gas: pressure, volume and temperature.
The equation is:
where
p is the pressure of the gas
V is the volume of the gas
n is the number of moles of the gas
R is the gas constant
T is the absolute temperature of the gas (must be expressed in Kelvin)
Here we want to solve the equation isolating p, the pressure of the gas.
We can do that simply by dividing both terms by the volume, V. We find:
So, we see that:
- The pressure is directly proportional to the temperature of the gas
- The pressure is inversely proportional to the volume of the gas
The product of reduction of ethyl 4-oxobutanoate with sodium borohydride in ethanol at room temperature for 30 minutes is ethyl 4- hydroxybutanoate .
Sodium borohydride is a relatively selective reducing agent Ethanolic solutions of Sodium borohydride reduces aldehyde , and ketone , in the presence of acid chloride , ester , epoxide , lactones , acids , nitriles , nitro groups.
The sodium borohydride does not reduce ester group because sodium borohydride is not strong enough and the electrophilicity at carbony carbon of ester is not more as compare toaldehyde , and ketone
The product of reduction of ethyl 4-oxobutanoate with sodium borohydride in ethanol at room temperature for 30 minutes is ethyl 4- hydroxybutanoate .
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27*9=243 if one mole is equal to 27 grams times that by 9
