95 grams of carbon dioxide equal 2.15 moles. This can be found using Avogadro's number (6.02 x 10^23)
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Explanation: bahahahahahahahahahahahahahahaha no
Answer:
73.2g
Explanation:
The reaction expression is given as:
P₄ + 6Cl₂ → 4PCl₃
Given parameters:
Volume of chlorine gas = 79.2L
Unknown:
Mass of Phosphorus needed = ?
Solution:
To solve this problem, let us find the number of moles of the chlorine gas.
Since the condition of the reaction is at STP;
22.4L of gas is contained in 1 mole
79.2L of chlorine gas will contain
= 3.54mole
From the reaction expression;
6 moles of chlorine gas will react with 1 mole of P₄
3.54 mole of chlorine gas will completely react with
= 0.59mole of P₄
Mass of P₄ = number of moles x molar mass
Molar mass of P₄ = 4 x 31 = 124g/mol
Mass of P₄ = 0.59 x 124 = 73.2g
Answer:
0.11M
Explanation:
What is the Molarity of a Ca(OH)2 solution if 30.0mL of
the solution is neutralized by 26.4mL of 0.25M HCI solution?
1L (1000 ml) of the HCl contains 0.25 moles of H ion
26.4 ml contains ( 26.4 X0.25/1000) moles of H ion ion
=0.0066 moles H ion
2HCl +Ca (OH)2-----> 2H2O +CaCl2
SO 2 H IONS NEUTRALIZE 1 Ca(OH)2 MOLECULE
00066 moles H ion neutralize 0.0033 moles Ca(OH)2
the 0.0033 moles are distributed over 30 ml, so the concentration of the
Ca(OH)2 IS 0,0033/(30/1000) =0.11 moles/liter or 0.11M
Answer:
There are 14.2 moles of carbon in 170.3 grams of carbon
Explanation:
The mass of one mole of carbon is known as the molar mass of carbon. the unit of molar mass is grams/mole, g/mol.
The molar mass of carbon is 12 grams. This means that for every 12 grams of carbon, one has one mole of carbon.
To determine the number of moles of carbon present in 170.3 grams of carbon, the given mass of carbon, that is 170.3 grams is divided by 12.
The formula to use is: number of moles = mass of substance/molar mass of substance
Number of moles of carbon = 170.3 g / 12 g/mol = 14.2 moles
Therefore, there are 14.2 moles of carbon in 170.3 grams of carbon