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3 years ago

Which elements are included in group 5a

Chemistry

1 answer:

RUDIKE [14]3 years ago

7 0

Answer:

Group 5A (or VA) of the periodic table are the pnictogens:

the nonmetals nitrogen (N),

and phosphorus (P),

the metalloids arsenic (As)

antimony (Sb),

the metal bismuth (Bi).

and moscovium (Mc).

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How many moles of c6h12o6 are consumed if 6 moles of o2 are consumed

Mrac [35]

C₆H₁₂O₆, or glucose, is oxidized in the presence of oxygen to form carbon dioxide and water. The reaction equation for this is:
C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O
Therefore, if 6 moles of oxygen are consumed, we can see from the equation that one mole of C₆H₁₂O₆ will be consumed.

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3 years ago

For the reaction, Cl2 + 2KBr --> 2KCl + Br2, how many moles of potassium chloride, KCl, are produced from 102g of potassium b

Sedaia [141]

Solution :

From the balanced chemical equation, we can say that 1 moles of KBr will produce 1 moles of KCl .

Moles of KBr in 102 g of potassium bromide.

n = 102/119.002

n = 0.86 mole.

So, number of miles of KCl produced are also 0.86 mole.

Mass of KCl produced :

$m = 0.86 \times Molar \ mass \ of \ KCl\\\\m = 0.86 \times 74.5 \ gram \\\\m = 64.07\ gram$

Hence, this is the required solution.

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3 years ago

If thermal energy (heat) must be added to a chemical reaction in order for the reaction to take place, the reaction is _________

Harlamova29_29 [7]

<span>If thermal energy (heat) must be added to a chemical reaction in order for the reaction to take place, the reaction is endothermic. </span>

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3 years ago

How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at a pressure of 12.4 atm and a tempe

polet [3.4K]

First, we need the no.of moles of O2 = mass/molar mass of O2
= 55 g / 32 g/mol
= 1.72 mol
from the balanced equation of the reaction:
2H2 (g) + O2(g) → 2H2O(g)
we can see that the molar ratio between O2: H2O = 1: 2
So we can get the no.of moles of H2O = 2 * moles of O2
= 2 * 1.72 mol
= 3.44 mol
So by substitution by this value in ideal gas formula:
PV = nRT

when P = 12.4 atm & n H2O = 3.44 mol & R= 0.0821 & T = 85 + 273=358K

12.4 atm *V = 3.44 * 0.0821 * 358 = 8.15 L
∴ V ≈ 8.2 L

4 0

4 years ago

How many liters of hydrogen gas will be produced at STP from the reaction of 7.179 x 1023 atoms of magnesium with 54.21 g of pho

wlad13 [49]

<h3>Answer:</h3>

18.58 liters of hydrogen gas

<h3>Explanation:</h3>

We are given;

The equation;

3Mg + 2H₃(PO₄) → Mg₃(PO₄)₂ + 3H₂

Atoms of Magnesium = 7.179 x 10^23 atoms
Mass of phosphoric acid as 54.21 g

We are required to determine the volume of hydrogen gas produced;

Step 1; moles of Magnesium

1 mole of an element contains 6.02 × 10^23 atoms

therefore;

Moles of Mg = (7.179 x 10^23 ) ÷ (6.02 × 10^23)

= 1.193 moles

Step 2: Moles of phosphoric acid

moles = Mass ÷ Molar mass

Molar mass of phosphoric acid = 97.994 g/mol

Therefore;

Moles of Phosphoric acid = 54.21 g ÷ 97.994 g/mol

= 0.553 moles

Step 3: Determine the rate limiting reagent

From the mole ratio of Mg to Phosphoric acid (3 : 2);

1.193 moles of magnesium requires 0.795 moles of phosphoric acid while,

0.0553 moles of phosphoric acid requires 0.8295 moles of Mg

Therefore, phosphoric acid is the rate limiting reagent

step 4: Determine the moles of hydrogen produced

From the equation, w moles of phosphoric acid reacts to produce 3 moles of hydrogen;

Therefore; moles of Hydrogen = moles of phosphoric acid × 3/2

= 0.553 moles × 3/2

= 0.8295 moles

Step 5: Volume of hydrogen gas

1 mole of a gas occupies a volume of 22.4 liters at STP

Therefore;

Volume of Hydrogen = 0.8295 moles × 22.4 L/mol

= 18.58 Liters

Therefore; 18.58 liters of hydrogen gas will be produced

4 0

3 years ago