What is the sum of the fractions 2/9+5/9

Is there any Way to Help with balancing Equations? i have been doing horrible with them

aleksandr82 [10.1K]

Yes there is a great way to balance equation s

6 0

3 years ago

3. What is the formula for the compound formed from the magnesium ion and nitrate?

bija089 [108]

Answer:

D.) Mg(NO₃)₂

Explanation:

Since magnesium (Mg) is a metal and nitrate (NO₃) is a polyatomic anion, they would combine to form an ionic compound. Magnesium would form the cation Mg²⁺ because it generally has 2 valence electrons. Nitrate always has a -1 charge.

In order for the overall compound to be neutral (have a charge of 0), there must be one Mg²⁺ and two NO₃⁻ ions in the compound (+2 + (-1) + (-1) = 0).

Therefore, the formula for the compound formed is Mg(NO₃)₂.

8 0

2 years ago

I need this answered!!For a testtt!!!!!!!

DanielleElmas [232]

I can’t see the question

7 0

3 years ago

A mixture of 0.2000 mol of CO2, 0.1000 mol of H2 and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium

Slav-nsk [51]

Answer:

a) p(CO2) = 4.103 atm

p(H2) = 2.0515 atm

p(H2O) = 3.2824 atm

b) pCO2 = 3.8754 atm

pH2 = 1.8239 atm

pCO = 0.2276 atm

pH2O = 3.51 atm

c) Kp= 0.113

Explanation:

Step 1: Data given

Moles of CO2 = 0.2000 mol

Moles of H2 = 0.1000 mol

Moles of H2O = 0.1600 mol

Volume = 2.000 L

Temperature = 500 k

Step 2: The balanced equation

CO2 (g) + H2 (g) → CO (g) + H2O (g)

Step 3: Calculate the initial partial pressures of CO2, H2, and H2O.

pV = nRT

P = (nRT)/V

p(CO2) = (0.2000 mol * 0.08206 * 500)/2.000L

⇒ p(CO2) = 4.103 atm

p(H2) = (0.1000 mol * 0.08206 * 500)/2.000L

⇒ p(H2) = 2.0515 atm

p(H2O) = (0.1600 mol * 0.08206 * 500)/2.000L

⇒ p(H2O) = 3.2824 atm

b. At equilibrium PH2O= 3.51 atm. Calculate the equilibrium partial pressures of CO2, H2, and CO.

Step 1: Calculate the change in pH2O

The change in pH2O = 3.51 - 3.2824 = 0.2276

Step 2: the initial pressures

pCO2 = 4.103 atm

pH2 = 2.0515 atm

pCO = 0 atm

pH2O = 3.2824

Step 3: The partial pressure at the equilibrium

Since there reacts 0.2276 atm for H2O, and the mol ratio is 1:1:1:1

For each gas, there will react 0.2276 atm

pCO2 = 4.103 - 0.2276 = 3.8754 atm

pH2 = 2.0515 - 0.2276 = 1.8239 atm

pCO = 0 + 0.2276 = 0.2276 atm

pH2O = 3.51 atm

c. Calculate Kp for this reaction

Kp = (pCO * pH2O)/ (pCO2 * pH2)

Kp = (0.2276 * 3.51) /( 3.8754 *1.8239)

Kp = 0.113

5 0

3 years ago

Dinitrogen tetroxide and hydrazine (N2H4) undergo a redox reaction in which nitrogen and water are formed as products. What mass

pantera1 [17]

Answer:

The mass of nitrogen molecule $N_2$ = 45.65 g

Explanation:

The equation for the redox reaction can be represented as follows:

$\mathtt{2N_2H_4 +N_2O_4 \ \to \ 3N_2 + 4H_2O}$

We know that:

numbers of moles = mass/molar mass

For $\mathtt{N_2O_4}$ :

number of moles = 50g/92 g/mol

number of moles = 0.5435 mol

For $\mathtt{N_2H_4}$ :

number of moles = 45 g/ 32 g/mol

number of moles = 1.40625 mol

From the above equation;

number of moles of $\mathtt{N_2O_4}$ needed = 1/2 moles of $\mathtt{N_2H_4}$ = 1/2 × 1.40625 mol

= 0.703125 mol

The amount of $\mathtt{N_2O_4}$ present = 0.5435 moles which is less than the needed. As such $\mathtt{N_2O_4}$ is the limiting reagent

The number of moles of nitrogen molecule $N_2$ produced = 3 × ( $\mathtt{N_2O_4}$ )

= 3 × 0.5435

= 1.6305 mol

The mass of nitrogen molecule $N_2$ = number of moles of $N_2$ × molar mass of $N_2$

The mass of nitrogen molecule $N_2$ = 1.6305 mol × 28 g/mol

The mass of nitrogen molecule $N_2$ = 45.654 g

The mass of nitrogen molecule $N_2$ = 45.65 g

7 0

3 years ago