<span>To solve this exercise you need to know that to create CO₂ with C₂H₂ is necessary to have oxygen. So, the following balanced equation represents the reaction:
2C₂H₂(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(g)
Notice that 2 moles of C₂H₂ form 4 moles of </span><span>CO₂, so if </span>3.3 moles of C₂H₂ react, how many moles of CO2 would be produced?
2 moles <span>of C₂H₂ -------</span>4 moles of <span>CO₂
3.3 </span><span>moles <span>of C₂H₂--------x moles of CO₂
x=6.6 </span></span><span>moles of CO₂ produced.</span>
Answer:
Alpha decay
Explanation:
That's the definition of alpha decay
Answer:
Neutron does not contain any charge because the charge of the quarks that made up the neutron balances each other out.
Hope it helps.
Answer:- partial pressure of Kr = 0.306 atm, partial pressure of oxygen = 0.264 atm and partial pressure of carbon dioxide = 0.396 atm
Total pressure is 0.966 atm
Solution:- moles of Kr = 21.7 g x (1mol/83.8g) = 0.259 mol
moles of oxygen = 7.18 g x (1mol/32g) = 0.224 mol
moles of carbon dioxide = 14.8 g x (1mol/44g) = 0.336 mol
Volume of container = 23.1 L and the temperature is 59 + 273 = 332 K
From ideal gas law equation, P = nRT/V
partial pressure of Kr = (0.259 x 0.0821 x 332).23.1 = 0.306 atm
partial pressure of oxygen = (0.224 x 0.0821 x 332)/23.1 = 0.264 atm
partial pressure of carbon dioxide = (0.336 x 0.0821 x 332)/23.1 = 0.396 atm
Total pressure of the gas mixture = 0.306 atm + 0.264 atm + 0.396 atm = 0.966 atm
