Alice has type A blood and her husband Mark has Type B blood

Balance and find out the coefficients of reactions and products

kolezko [41]

Answer:

2, 1, 1, 4.

Explanation:

Hello there!

In this case, for the given chemical reaction:

$H_2SO_4+Pb(OH)_4\rightarrow Pb(SO_4)_2+H_2O\\$

We can see how there is one SO4 on the left and two on the right, thus, we add a 2 in front of H2SO4:

$2H_2SO_4+Pb(OH)_4\rightarrow Pb(SO_4)_2+H_2O\\$

Next, since there are 8 atoms of hydrogen on the left and two on the right, we add a 4 in front of H2O to obtain:

$2H_2SO_4+Pb(OH)_4\rightarrow Pb(SO_4)_2+4H_2O\\$

Which is now balanced so the coefficients 2, 1, 1, 4.

Best regards!

6 0

2 years ago

Which term best describes what Donna observed? A:dew B:fog C:mist D:rain

MariettaO [177]

I also think it’s B but not quite sure

6 0

3 years ago

A student balanced the chemical equation Mg + O2 →MgO by writing Mg + O2 → MgO2. Was the equation balanced correctly? Explain yo

Amanda [17]

Explanation:

Charges on both magnesium and oxygen is 2. Though opposite in sign, they have equal charges so, both of them will be cancelled by each other.

As a result, formula of magnesium oxide is MgO and not $MgO_{2}$ .

The student write the equation as $Mg + O_2 \rightarrow MgO_2$ , it is not correct.

Therefore, given equation will be balanced as follows.

$2Mg + O_{2} \rightarrow 2MgO$

Since, number of atoms on both reactant and product side are equal. Hence, this equation is completely balanced.

7 0

3 years ago

200.00 grams of an organic compound is known to contain 83.884 grams of carbon, 10.486

ololo11 [35]

The empirical formula of a given compound is C6H9ON5.

Explanation:

Step 1: Obtain the mass of each element present in grams

Element % = mass in g = m

Carbon = 83.884 grams, Hydrogen = 10.486 grams, Oxygen = 18.640 grams, Nitrogen = 86.99 grams.

Step 2: Determine the number of moles of each type of atom present

m/atomic mass = Molar amount (M)

Molar amount of carbon = (83.884 1 mol ) / 12 g = 6.99

Molar amount of hydrogen = (10.486 1 mol) / 1 g = 10.49

Molar amount of oxygen = (18.64 1 mol) / 16 g = 1.17

Molar amount of nitrogen = (86.99 1 mol) / 14 g = 6.21

Step 3: Divide the number of moles of each element by the smallest number of moles

M / least M value = Atomic Ratio (R)

Atomic radius of carbon = 6.99 / 1.17 = 5.9 = 6

Atomic radius of hydrogen = 10.49 / 1.17 = 8.9 = 9

Atomic radius of oxygen = 1.17 / 1.17 = 1

Atomic radius of nitrogen = 6.21 / 1.17 = 5

Step 4: Convert numbers to whole numbers. This set of whole numbers are the subscripts in the empirical formula.

R * whole number = Empirical Formula

The empirical formula of a given compound is C6H9ON5.

7 0

3 years ago

Stemscopedia

Alexeev081 [22]

What’s the question

7 0

3 years ago