The volume in liters occupied by 22.6 g of I₂ gas at STP is 1.99 L (answer A)
<u><em>calculation</em></u>
Step: find the moles of I₂
moles= mass÷ molar mass
from periodic table the molar mass of I₂ is 253.8 g/mol
moles = 22.6 g÷253.8 g/mol =0.089 moles
Step 2:find the volume of I₂ at STP
At STP 1 moles =22.4 L
0.089 moles= ? L
<em>by cross multiplication</em>
={ (0.089 moles x 22.4 L) /1 mole} = 1.99 L
For this, you need to know 1) the mass of the hydrate and 2) the mass of the anhydrous salt. Once you have both of these, you will subtract 1) from 2) to find the mass of the water lost.
From the problem, you know that 1) = 2.000 g.
Now you need to find 2). You know that your crucible+anhydrous salt is 5.022 g. To find just the anhydrous salt, subtract the mass of the crucible (3.715 g).
1) = 5.022 g - 3.715 g = 1.307 g
Now you can complete our original task.
Mass H2O = 2) - 1) = 2.000 g - 1.307 g = 0.693 g.
Answer:
An endothermic reaction
Explanation:
A positive sign indicates that energy is absorbed. Hence it is an endothermic reaction.
A reversible reaction is indicated by a double arrow on the chemical equation.
A spontaneous is indicated by negative Gibbs Free Energy (G) value.
An exothermic reaction is indicated by a negative enthalpy change
Answer:
1.1grams
Explanation:
Find moles of water:
4.5x10^22/(6.02x10^23)=0.07mol
Find molar mass of the water
O=16.00g/mol
0.07x 16.00=1.1 grams
True
Explanation: Covalent bonds occur when electrons are shared between two atoms. A single covalent bond is when only one pair of electrons is shared between atoms.
