What element is this?

Which is an example of diffraction?

jeyben [28]

I would say d but I’m not sure

8 0

3 years ago

WHAT MASS OF WATER WILL BE PRODUCED FROM 2.70 MOLES OF CA(OH)2 REACTING WITH HCI

Keith_Richards [23]

<u>Answer:</u> The mass of water produced in the reaction is 97.2 grams

<u>Explanation:</u>

We are given:

Moles of calcium hydroxide = 2.70 moles

The chemical equation for the reaction of calcium hydroxide and HCl follows:

$Ca(OH)_2+HCl\rightarrow CaCl_2+2H_2O$

By Stoichiometry of the reaction:

1 mole of calcium hydroxide produces 2 moles of water

So, 2.70 moles of calcium hydroxide will produce = $\frac{2}{1}\times 2.70=5.40mol$ of HCl

To calculate mass for given number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Molar mass of water = 18 g/mol

Moles of water = 5.40 moles

Putting values in above equation, we get:

$5.40mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=(5.40mol\times 18g/mol)=97.2g$

Hence, the mass of water produced in the reaction is 97.2 grams

3 0

4 years ago

hola genteee ayuda me pueden decir 5 propiedades físicas y 5 propiedades químicas del ácido sulfúrico porfa es urgente !

Alexus [3.1K]

Answer:

La respuesta está en la explicación.

Explanation:

Las propiedades físicas son las visibles y medibles que no afectan químicamente la sustancia en cuestión. Las propiedades químicas hacen alusión a la reactividad de la sustancia:

Propiedades físicas ácido sulfúrico:

Líquido a temperatura ambiente.

Densidad: 1.83g/mL

Punto de fusión: 10°C

Punto de ebullición: 337°C

Índice de refracción: 1.397

Propiedades Químicas:

Ácido Fuerte.

Oxidante Fuerte.

Miscible con el agua reaccionando exotérmicamente.

A temperaturas > 30°C produce vapores azufrados.

Estable en concentraciones menores al 98%

8 0

4 years ago

A laboratory experiment requires 4.8 l of a 2.5 m solution of sulfuric acid (h2so4), but the only available h2so4 is a 6.0 m sto

Airida [17]

To determine the amount of 6.0 M H2SO4 needed for the preparation, equate the number of moles of the 6.0 M and 2.5 M H2SO4 solution. This is done as follows

M1 x V1 = M2 x V2

Substituting the known variables,

(6.0 M) x V1 = (2.5 M) x (4.8 L)

Solving for V1 gives an answer of V1 = 2 L. Thus, to prepare the needed solution, dilute 2 L of 6.0 M H2SO4 solution with water until the volume reach 4.8 L.

5 0

4 years ago

Read 2 more answers

2Ag (s) + H2S(s) → Ag2S(s) + H2(g)

Advocard [28]

Answer: Oxidation half: $2Ag\rightarrow 2Ag^++2e^-$