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3 years ago

Which element can form an oxide with the general formula m2o or mo where m is a metal

Chemistry

1 answer:

boyakko [2]3 years ago

7 0

Answer:

Because the compound has a formula of M2O, the number of valence electrons of M should be 1. Therefore, (1) Group 1 is the correct answer because elements in group 1 have 1 valence electron.

Explanation:

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When both –NH2 and –COOH replace hydrogen atoms on the same carbon atom, a(n) ____ is formed. a. amine c. carboxylic acid b. ami

Mice21 [21]

$-NH_{2}$ represents amine functional group and $COOH$ represents carboxylic acid functional group. When these both functional groups are substituted onto a single carbon atom, then amino acid is formed.

The organic compound consists of $-NH_{2}$ functional group and $COOH$ functional group with a side chain is said to be an amino acid.

A: amine group is $-NH_{2}$ .

C: carboxylic acid group is $COOH$

B: amino acid represents $-NH_{2}$ functional group and $COOH$ functional group which are substituted onto a single carbon atom.

D: carbohydrate: the general formula of carbohydrate is $(CH_{2} O)_{x}$ .

Hence, amino acid is the correct answer.

4 0

3 years ago

Which of the following most likely happens when the volume of a gas increases the number of collisions of gas particles remains

lord [1]

When the collision of gas particles and the volume of the gas stay the same it causes a chemical.

5 0

3 years ago

Read 2 more answers

A 12.0 g sample of a metal is heated to 90.0 ◦C. It is then dropped into 25.0 g of water. The temperature of the water rises fro

deff fn [24]

Answer:

The specific heat of the metal is 0.34 J/g°C

Explanation:

Step 1: Data given

Mass of the metal = 12.0 grams

Mass of the water = 25.0 grams

Initial temperature of the metal = 90.0 °C

Initial temperature of the water = 22.5 °C

Final temperature = 25 °C

Specific heat of water = 4.184 J/g°C

Step 2: Calculate the specific heat of the metal

Qlost = Qgained

Q = m*c*ΔT

Qmetal = -Qwater

m(metal) *c(metal)* ΔT(metal) = -m(water) * c(water) *ΔT(water)

⇒ with mass of metal = 12.0 grams

⇒ with c(metal) = TO BE DETERMINED

⇒ with ΔT(metal) = T2 - T1 = 25.0°C - 90.0 °C = -65.0 °C

⇒ with mass of water = 25.0 grams

⇒ with c(water) = 4.184 J/g°C

⇒ with ΔT(water) = T2 - T1 = 25.0 - 22.5 °C = 2.5 °C

12.0 * c(metal) * -65.0 °C = -25.0g * 4.184 J/g°C * 2.5°C

-780.0 * c(metal) = -2615 ( 2.6*10^3 with sig figs)

c(metal) = 0.335 (=0.34 with sig figs)

The specific heat of the metal is 0.34 J/g°C

3 0

3 years ago

For the following gases, correct the volumes to the conditions indicated. A.654 cm3 at 6 degrees Celsius and 65.3 kPa to 4 degre

leva [86]

Initial pressure of the gas = 65.3 kPa

Initial volume of the gas = 654 cm³

Initial temperature of the gas = 6⁰C = 273 + 6 = 279 K

Final pressure of the gas = 108.7 kPa

Final temperature of the gas = 4⁰C = 273 + 4 = 277 K

Using the combined gas law for ideal gases:

P₁V₁/T₁ = P₂V₂/T₂

where P₁, V₁ and T₁ are the pressure, volume and temperature for the initial state and P₂, V₂ and T₂ are the pressure, volume and temperature for the final state.

Plugging the given data into the combined gas law we have,

(65.3 kPa x 654 cm³) / (279 K) = (108.7 kPa x V₂)/(277 K)

V₂ = (65.3 kPa x 654 cm³ x 277 K) / (279 K x 108.7 kPa)

V₂ = 390.1 cm³

8 0

3 years ago

According to the following reaction, how many grams of hydrogen peroxide (H2O2) are needed to form 32.0 grams of oxygen gas?

Nesterboy [21]

Answer:

The answer to your question is 34 g of H₂O₂

Explanation:

Data

mass of H₂O₂ = ?

mass of O₂ = 32 g

Process

1.- Write the balanced chemical reaction

H₂O₂ ⇒ H₂ + O₂

2.- Calculate the molar mass of H₂O₂ and O₂

Molar mass H₂O₂ = (1 x 2) + (16 x 2) = 34 g

Molar mass of O₂ = 2 x 16 = 32 g

3.- Use proportions to calculate the mass of O₂

34g of H₂O₂ -------------- 32g of O₂

x -------------- 32g of O₂

x = (32 x 34) / 32

x = 34 g of H₂O₂

5 0

3 years ago