Answer:
Explanation: It is already known that 1 mole of the gas( or 32g of O2) is equivalent to 22.4 Litres of the oxygen gas. So, 8g is equivalent to = (22.4/32) × 8 = 5.6 L of the gas.
Answer:
![P_2=1.90atm](https://tex.z-dn.net/?f=P_2%3D1.90atm)
Explanation:
Hello!
In this case, according to the ideal gas equation ratio for two states:
![\frac{P_1V_1}{P_2V_2} =\frac{n_1RT_1}{n_2RT_2}](https://tex.z-dn.net/?f=%5Cfrac%7BP_1V_1%7D%7BP_2V_2%7D%20%3D%5Cfrac%7Bn_1RT_1%7D%7Bn_2RT_2%7D)
Whereas both n and R are cancelled out as they don't change, we obtain:
![\frac{P_1V_1}{P_2V_2} =\frac{T_1}{T_2}](https://tex.z-dn.net/?f=%5Cfrac%7BP_1V_1%7D%7BP_2V_2%7D%20%3D%5Cfrac%7BT_1%7D%7BT_2%7D)
Thus, by solving for the final pressure, we obtain:
![\frac{P_2V_2}{P_1V_1} =\frac{T_2}{T_1}\\\\P_2=\frac{T_2P_1V_1}{V_2T_1}](https://tex.z-dn.net/?f=%5Cfrac%7BP_2V_2%7D%7BP_1V_1%7D%20%3D%5Cfrac%7BT_2%7D%7BT_1%7D%5C%5C%5C%5CP_2%3D%5Cfrac%7BT_2P_1V_1%7D%7BV_2T_1%7D)
Now, since initial conditions are 1.00 atm, 273.15 K and 17 L and final temperature and volume are 94 + 273 = 367 K and 12 L respectively, the resulting pressure turns out to be:
![P_2=\frac{367K*1.00atm*17L}{12L*273.15K}\\\\P_2=1.90atm](https://tex.z-dn.net/?f=P_2%3D%5Cfrac%7B367K%2A1.00atm%2A17L%7D%7B12L%2A273.15K%7D%5C%5C%5C%5CP_2%3D1.90atm)
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Answer:
A. True
B. False
Explanation:
Reaction between hypochlorous acid and ammonia does not yields a Ph value of 7.00 , this value is defined to water and no other reaction can yield exactly this Ph value. The acid reaction will give a Ph value below 7 while a base reaction will give Ph value of above 7.
Does the element have a different amount of electrons than protons?