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3 years ago

Which set of coefficients would balance the following chemical equation? H3PO4 + RbOH → H2O + Rb3PO4

Chemistry

2 answers:

AleksandrR [38]3 years ago

5 0

H3PO4 + 3RbOH > 3H20 + Rb3PO4

ankoles [38]3 years ago

4 0

Answer:

The balanced equation is:

$H_3PO_4 + 3 RbOH \longrightarrow 3 H_2O +Rb_3PO_4$

Explanation:

Hi, step by step:

1) Balance the Rb:

$H_3PO_4 + 3 RbOH \longrightarrow H_2O +Rb_3PO_4$

2) Balance the phosphate:

$1 H_3PO_4 + 3 RbOH \longrightarrow H_2O +Rb_3PO_4$

3) Balance the water:

$1 H_3PO_4 + 3 RbOH \longrightarrow 3 H_2O +Rb_3PO_4$

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Can i have sum help pls :)

Phantasy [73]

Answer:

LOL the word is some and not "sum"

4 0

2 years ago

When 28 g of nitrogen and 6 g of hydrogen react, 34 g of ammonia are produced. If 100 g of nitrogen react with 6 g of hydrogen,

love history [14]

Answer:

34 g

Explanation:

Let's consider the following balanced equation.

N₂ + 3 H₂ → 2 NH₃

The theoretical mass ratio of N₂ to H₂ is 28g N₂ : 6g H₂ = 4.6g N₂ : 1g H₂.

The experimental mass ratio of N₂ to H₂ is 100g N₂ : 6g H₂ = 16.6g N₂ : 1g H₂.

As we can see, hydrogen is the limiting reactant.

According to the task, we 6 g of H₂ react completely, 34 g of ammonia are produced.

3 0

3 years ago

The number placed in front of a compound to balance a chemical reaction is called

masha68 [24]

Answer: The number placed in front of a compound to balance a chemical reaction is called coefficient.

Explanation:

Assume this general form for a chemical equation:

aA + bB → cC + dD

The letters a, b, c, and d, in front of each compound A, B, C, and D, are called coefficients and indicate the number of formula units (molecules or ions) that take part in the equation.

Those coefficients are needed to balance the equation and ensure compliance with the law of mass conservation.

This example shows it:

Word equation: hydrogen + oxygen yields water

Chemical equation: H₂ (g) + O₂(g) → H₂O(g)

Balance, adding the coefficients so that the number of each kind of atoms is the same on the left and the right of the chemical equation:

H₂ (g) + 2O₂(g) → 2H₂O(g)

In that equation:

The coefficient of H₂ (g) on the left is 1 (it is not written)

The coefficient of O₂(g) on the left is 2

The coefficient of H₂O(g) on the right is 2

You read it as: 1 mole of gaseous hydrogen and 2 moles of gaseous oxygen yield 2 moles of water vapor.

4 0

3 years ago

What is the total mass of NaNO3 that must be added to 70g in 100 grams of H2O to make a saturated solution at 30°C ?

dimulka [17.4K]

Answer:

58g

Explanation:

In order to solve this problem, you must take a look at the solubility graph for potassium nitrate.

Now, the solubility graph shows you how much solute can be dissolved per 100g of water in order to make an unsaturated, a saturated, or a supersaturated solution.

You're looking to make a saturated potassium nitrate solution using

50g of water at 60∘C. Your starting point will be to determine how much potassium nitrate can be dissolved in 100g of water at that temperature in order to have a saturated solution.

As you can see, the curve itself represents saturation.

If you draw a vertical line that corresponds to 60∘C and extend it until it intersects the curve, then draw a horizontal line that connects to the vertical axis, you will find that potassium has a solubility of about

115g per 100g of water. Your answer is 58g of potassium nitrate

7 0

4 years ago

_S8+ _02 - SO3

Anton [14]

Answer:

a) $S_8+12O_2\rightarrow 8SO_3$

b) Combination or synthesis reaction

$1molS_8:12molO_2;or\\ \\ \\ \dfrac{1molS_8}{12molO_2}$

d) 30 g.

Explanation:

a. Balance the Equation

To balance the equation you must add the coefficients that yield the same number of atoms for the same kind of atoms on each side of the chemical equation.

You cannot modify the superscripts because the they are part of the chemical formula of the compound or molecule, they indicate the number of atoms of each kind inside the compound, i.e. they determine the composition substance.

The coefficients can be adjusted because they just indicate the number of units that react or are produced.

Starting from the skeleton equation:

$S_8+O_2\rightarrow SO_3$

Add an 8 before the SO₃ to balance the S atoms:

$S_8+O_2\rightarrow 8SO_3$

Now add a coefficient of 12 for the O₂ molecule on the left side:

$S_8+12O_2\rightarrow 8SO_3$

If you count:

Atom Leff side Right side

S 8 8

O 24 24

Thus, the equation is balanced.

b. What type of chemical reaction is this?

When two elements or compounds combine to form one single compound that is a combination reaction.

The general form of a combination reaction is:

A + B → AB

This is called comibnation to distinguish from single replacement, double replacement, decompositon, and combustion reaction.

It is also named synthesis reaction because a new compound is being synthetized ("created") from simpler substances.

The combination of a non-metal and oxygen is a typical reaction of synthesis in which a basic oxide is produced. They are named basic oxides because they react with water to form a base: hydroxide.

c. What is the molar ratio of S₈, to O₂?

The mole ratio also called theoretical or stoichiometric mole ratio is the ratio of coefficients of the substances. The mole ratio of the reactants indicate the proportion in which the reactants combine to each other to form the product or products.

Then, take the coefficients of S₈ and O₂ from the balanced molecular chemical equation and form the ratio:

$1molS_8:12molO_2;or\\ \\ \\ \dfrac{1molS_8}{12molO_2}$

That means that every molecule (or mole of molecules) of S₈ reacts with 12 molecules (or mole of molecules) of O₂ to form the products: in this case 8 molecules (or mole of molecules of SO₃).

You use this ratio to determine the yield of the reactions in a procedure called stoichiometric calculations.

d. How many grams of O₂ should be used if 100 grams of SO₃, is the desired end product?

You will need the mole ratio of O₂ to SO₃ and the molar masses of both substanes.

Mole ratio:

$\dfrac{8molSO_3}{12molO_2}$

Moles of SO₃

moles = mass in grams/molar mass

molar mass of SO₃ = 80.066g/mol

moles of SO₃ = 100g / 80.066g/mol = 1.25 mol SO₃

Moles of O₂

$1.25molSO_3\times 12molO_2/8molSO_3=1.875molO_2$

Conver to mass of O₂

molar mass of O₂ = 15.999 g/mol

mass of O₂ = 1.875mol × 15.999g/mol = 29.998 g

Round to 1 significant figures: 30 g.

6 0

3 years ago